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Derive the relationship between the constants a and b of the Dieterici equation: p=(RT/V-b)exp(-a/RTV)
Determine hydroxyl and hydrogen ion concentration in this solution. (if Ka for ammonium ion = 5.0 x 10^-10.)
When heated, hydrogen sulfide gas decomposes according to the equation above. A 4.40 g sample of H2S(g) is introduced into an evacuated rigid 1.50 L container. The sealed container is heated to 583 K and 5.72x10^-2 mol of S2(g) is present at equil..
what mass spectrometry techniw would be most effective in determining the chemical structure?
Calculate the percent ionization of propionic acid (C2H5COOH) in solutions of each of the following concentrations
the chromatographic paper in the spot testing chromatogram. predict the effect of this procedural change on the solution of the cation in the standard mixture
Classify each of the following reactions as combination, decomposition, single replacement, or double replacement: a) CuO(s)+2HCl(aq)-->CuCl2(aq)+H2O(l); b) 2Al(s)+3Br2(g)-->2AlBr3(s); c)Pb(NO3)2(aq)+2NaCl(aq)-->PbCl2(s)+2NaNO3(aq); d)2Mg(s)+O2(g..
How many Carbon 14 atoms are in a charcoal sample that has a decay rate of 3500 disintegrations per min
12.0 moles of gas are in a 6.00 tank at 20.3. Calculate the difference in pressure between methane and an ideal gas under these conditions. The van der Waals constants for methane are a=2.300 L^2*atm/mol^2 and b=0.0430 L/mol .
Pure metals are commonly recovered from sulfide ores by successive processes of roasting in air (oxidation), dissolution in sulfuric acid and electrolysis (reduction). Consider the starting ore mineral sphalerite (ZnS). Write balanced chemical rea..
Concetrated acedic acid is a Class II combustible liquid. What is the molecular weight of acetic acid that will form 2 moles of CO2 assuming complete combustion.
When an ant bites you, the reason it stings is because of an injection of formic acid. What is the pH when 50.0 mL of 0.1480 M formic acid (HCOOH) is titrated with 40.2 mL of 0.1841 M NaOH? PKa formic acid = 3.745.
58.0 mL of a 1.30 M solution is diluted to a volume of 228 mL. A 114-mL portion of that solution is diluted using 141 mL of water.
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